Valence Bond Theory and Orbital Hybridization Concepts

Covalent Bonding

Atoms share electrons to complete valence shells.

Valence Bond Theory

Atoms share electrons via overlapping atomic orbitals.

Atomic Orbitals

Regions of space where electrons are likely found.

Sigma Bond

Covalent bond from end-to-end orbital overlap.

Pi Bond

Covalent bond from sideways orbital overlap.

Single Bond

Consists of one sigma bond only.

Double Bond

One sigma bond and one pi bond.

Triple Bond

One sigma bond and two pi bonds.

Hybridization

Mixing atomic orbitals to form new orbitals.

sp Hybridization

One s and one p orbital combine, linear geometry.

sp² Hybridization

One s and two p orbitals combine, trigonal planar.

sp³ Hybridization

One s and three p orbitals combine, tetrahedral geometry.

sp³d Hybridization

One s, three p, and one d orbital, trigonal bipyramidal.

sp³d² Hybridization

One s, three p, and two d orbitals, octahedral geometry.

VSEPR Theory

Predicts molecular geometry based on electron repulsion.

Ethene

Example of sp² hybridization with double bond.

Methane (CH₄)

Example of sp³ hybridization with tetrahedral shape.

Bond Angle

Angle between adjacent bonds in a molecule.

Trigonal Planar

Geometry with bond angles of 120 degrees.

Tetrahedral Geometry

Geometry with bond angles of 109.5 degrees.

Overlap of p Orbitals

Forms pi bonds in multiple bonds.

Hybrid Orbitals

New orbitals formed from hybridization of atomic orbitals.

Bonding Electrons

Electrons involved in forming covalent bonds.